Which pair will form the most stable ionic bo | vedclass

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(C) The stability of an ionic bond is determined by the lattice energy of the resulting ionic compound.Lattice energy is directly proportional to the

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$Mg$ and $F$

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(C) The stability of an ionic bond is determined by the lattice energy of the resulting ionic compound.Lattice energy is directly proportional to the product of the charges of the ions and inversely proportional to the interionic distance $(U \propto \frac{q_1 q_2}{r_0})$.For $MgF_2$,the charges are $Mg^{2+}$ and $F^-$,giving a product of charges equal to $2 	imes 1 = 2$.For $NaF$,$LiF$,and $NaCl$,the product of charges is $1 	imes 1 = 1$.Since $MgF_2$ has a higher charge product and relatively small ionic radii,it possesses the highest lattice energy,making it the most stable ionic bond among the given options.

Which pair will form the most stable ionic bond?

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Assertion $(A)$: Higher lattice enthalpy leads to greater stability of ionic compounds.
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